Sr,Mg, and Ba are examples of what type of elements?
A)
halogens
B)
Alkali metals
C)
Transition metals
D)
Alkaline earth metals
3.
A compound made from tin II and fluorine has what formula?
A)
SnF
B)
Sn2F3
C)
Sn2F
D)
SnF2
4.
An ionic compound made from strontium and nitrogen has what formula?
A)
Sr2N
B)
Sr3N2
C)
N3Sr2
D)
SrN
5.
What is the correct formula of a compound made from carbonate and aluminum?
A)
Al2(CO3)3
B)
Al2CO3
C)
Al3C2
D)
CaAl2
6.
The acetate ion has what formula?
A)
C2H3O21–
B)
C2H3O23–
C)
CHO21–
D)
C2O21–
7.
What is the formula for tetranitrogen monoiodide?
A)
N4I
B)
NI4
C)
N4I4
D)
NI
8.
When electrons are shared between two atoms' outer electron shells, what kind of bond forms?
A)
an ionic bond
B)
a covalent bond
C)
a metallic bond
D)
a coordinate covalent bond
9.
A combustion reaction always has
A)
a hydrocarbon as a reactant
B)
always produces carbon dioxide and water
C)
reacts in the presence of oxygen
D)
all of the above
E)
a and b only
10.
A precipitation reaction always includes
A)
only liquid substances
B)
a solid as a reactant
C)
a solid as a product
D)
a gas
11.
The following reaction is a(n)__? Hg(NO3)2 (aq)+ HCl (aq) →HgCl2(s) +HNO3 (aq)
A)
combustion
B)
precipitation
C)
neutrilization
D)
oxidation
12.
The following, HCl (aq) + Ca(OH)2 (aq) → H2O (aq) + CaCl2(aq), qualifies as what type of reaction?
A)
an oxidation–reduction
B)
a precipitation
C)
an addition reaction
D)
a neutralization
SHORT ANSWER/ESSAY: Answer the following in the space provided.
13.
Balance the following equation: P+O2→P2O5
14.
Balance the following equation: NaBr +Fe2(CO3)3→Na2(CO3)+FeBr3
15.
Write a balanced equation for the following reaction: nickel and titanium (I) phosphate form titanium and nickel II phosphate .
16.
Predict the products of the following a. the combustion of octane (C8H18) and oxygen b. the neutralization of HF and CsOH .
17. Define the following terms and explain how they relate to each other: mole to mole ratio, limiting reactant and theoretical yield.
Problems: Show all work on the math problems. Circle the final answer. Be sure to use significant figures and units of measure in all answers.
18.
What is the mass in grams of 1.25 moles of platinum?
19.
What is the number of mole of 2.50 grams of Ag2O?
20.
A sample has 5.7 g of xenon. How many atoms are in this sample?
21.
How many moles of KF are in 3.2x1024 particles? .
22.
What is the theoretical yield in grams of carbon dioxide if 12.15 g of C2H6 are completely consumed, according to the balanced equation below: 2C2H6 + 7 O2 → 4CO2 + 6 H2O
23.
How many grams of sulfur are needed to react completely with 4.20 g of aluminum when aluminum reacts with sulfur to form aluminum sulfide?
24.
If 42.0 g of yttrium and 32.0 g of bromine are mixed according to the balanced equation 4 Y + 3Br2 → 2 Y2Br3 What is the theoretical yield in grams and which is the limiting reagent? .
25.
Barium reacts with hydrogen fluoride to form barium fluoride and hydrogen gas. What is the theoretical yield of barium fluoride in grams and what is the limiting reactant when 65.0 g of barium is mixed with 44.5 g HF?
Chapter 4 part I review
Multiple Choice: circle the best answer.
1.
What is the name of the column in the periodic table that includes Mg, Ca, and Sr?
A)
the main group metals
B)
the transition metals
C)
the alkaline earth metals
D)
the alkali metals
2.
Pt and Ta are atomic symbols for elements that fall into what group on the periodic table?
A)
transition metals
B)
outer transition metals
C)
inner transition metals
D)
main group metals
3.
Al and K are examples of what type of element?
A)
main group non-metals
B)
representative metals
C)
main group metals
D)
transition metals
4.
Cl, Br, and I are examples of what type of elements?
A)
halogens
B)
main group gases
C)
noble gases
D)
pnicogens
5.
What is the name of the ion, Mg2+?
A)
magnesium ion
B)
magnesium atom
C)
magneside ion
D)
magneside atom
6.
What is the proper name for I1–?
A)
the iodide ion
B)
the iodate ion
C)
the iodonium ion
D)
the iodic ion
7.
What is the correct formula of an ionic compound made only from sodium and oxygen?
A)
NaO
B)
Na2O
C)
NaO2
D)
Na2O2
8.
What formula does an ionic compound made from aluminum and chlorine have?
A)
AlCl2
B)
AlCl3
C)
Al2Cl
D)
Al3Cl
9.
What is the correct formula of an ionic compound made from phosphorus and calcium?
A)
CaP2
B)
Ca2P
C)
Ca3P2
D)
Ca2P3
10.
What formula does an ionic compound made from Cu2+ and nitrogen possess?
A)
CuN
B)
Cu3N2
C)
Cu2N3
D)
Cu3N3
11.
The sulfate ion has what formula?
A)
SO32–
B)
SO42–
C)
SO4–
D)
SO3–
12.
When electrons are shared between two atoms' outer electron shells, what kind of bond forms?
A)
an ionic bond
B)
a covalent bond
C)
a metallic bond
D)
a coordinate covalent bond
13.
What is the name of SF4?
A)
sulfur difluoride
B)
tetrasulfur fluoride
C)
tetrafluoro sulfide
D)
sulfur tetrafluoride
14.
Oxygen in nature has what formula?
A)
O3
B)
O4
C)
O
D)
O2
15.
The reactants of a chemical reaction are commonly listed where?
A)
in the middle of a chemical reaction
B)
on the left of a chemical reaction
C)
on the right of a chemical reaction
D)
at either end of a chemical reaction
16.
NO3 has what proper name?
A)
nitrogen dioxide
B)
nitrogen oxide
C)
nitrogen trioxide
D)
trinitrogen monoxide
17.
The give and take of electrons results in
A)
a covalent bond
B)
a metallic bond
C)
an ionic bond
D)
a polar covalent bond
18.
S2O3 has what proper name?
A)
sulfur dioxide
B)
disulfur trioxide
C)
trisulfur trioxide
D)
disulfate trioxide
SHORT ANSWER/ESSAY: Answer the following in the space provided.
19.
What is the name for P3Br2?
20.
What is the name for Cr2S3?
21.
What is the name of P2Cl4?
22.
Write the chemical formula for iron II nitrate. Identify the polyatomic ion if one is present.
23.
Dihydrogen monoxide has what chemical formula?
24.
Name the element with the lowest electronegativity.
25.
Discuss cations and anions and how they are used in naming.
26.
What is meant by the common names alcohol and salt?
27.
Identify the following:
The element located at period 2 and group 15.
Name two alkali metals
Name a halogen
What is the first element in period 6
28.
Which element has the higher melting point, NaBr or SBr? Explain.
29.
List two properties of ionic compounds and two properties of covalent compounds? How do these bonds differ?
30.
Balance the following:
KMnO4 →K2O+MnO+O2
N2+H2→NH3
Fe(OH)3 àFe2O3 +H2O
gold plus sulfur yields gold (I) sulfide
lithium plus water yields hydrogen plus lithium hydroxide
Chapter 3 review
(again, please note that the wiki will not do superscripts or subscripts) Multiple Choice: circle the best answer.
1.
DNA evidence cannot be used to identify remains in a funerary urn. Why?
A)
There is not enough DNA in the urn.
B)
Cremation destroys all DNA.
C)
There is no DNA in bones.
D)
Cremation doesn't burn body parts that contain DNA.
2.
The law of conservation of mass states:
A)
Mass is neither created nor destroyed in a chemical reaction, but merely changes state.
B)
Mass is neither created nor destroyed in a chemical reaction, but merely changes form.
C)
Mass is created or destroyed in a chemical reaction, while changing form.
D)
Mass and energy are neither created nor destroyed in a chemical reaction, but merely change form.
3.
Why does mass appear to be lost in a reaction involving burning in an open system?
A)
Matter escapes as a gas.
B)
Matter as ashes is smaller than the starting material.
C)
Matter is made less dense in the burning process.
D)
Burning causes the loss of matter.
4.
In a reaction, 54.0 g of HgO is heated, producing 43.0 g of mercury and g ofoxygen.
A)
97.0 g
B)
1.2 g
C)
11.0 g
D)
0.8 g
5.
Dalton's Atomic Theory states that all atoms of a given element are
A)
identical
B)
stable
C)
of the same mass
D)
of the same charge
6.
The observation that all samples of sodium always appear to be a metal is an example of what idea within Dalton's atomic theory?
A)
All matter is made up of tiny particles called atoms.
B)
All atoms of a given element are identical.
C)
Atoms combine in simple, whole number ratios.
D)
Atoms are neither created nor destroyed in a chemical reaction.
7.
How many protons are in all atoms of arsenic?
A)
32
B)
33
C)
74
D)
75
8.
The two compounds SO2 and SO3 are both made only from oxygen and sulfur. This is an example of which of Dalton's Laws?
A)
the law of conservation of mass
B)
the law of multiple proportions
C)
the atomic theory
D)
the law of conservation of charge
9.
Boron has how many protons?
A)
2
B)
3
C)
4
D)
5
10.
When an element has 12 neutrons and a Z = 12, what element and isotope are present?
A)
24/12Mg
B)
12/12Mg
C)
24/24Mg
D)
24/24Cr
11.
The isotope of cobalt with the symbol 59/27Co has how many neutrons?
A)
33
B)
32
C)
59
D)
27
12.
An atom of Fe contains how many electrons?
A)
25
B)
26
C)
55
D)
56
13.
Bromine is mostly two isotopes, neither of which is bromine-80.Which is the predominant one?
A)
82
B)
81
C)
79
D)
78
14.
An electron in an excited state has
A)
not absorbed energy
B)
absorbed a photon
C)
absorbed a quantum of energy
D)
moved closer to the nucleus
15.
What is the maximum number of electrons that can be contained in an orbital?
A)
6
B)
2
C)
10
D)
14
16.
A material uniformly containing 30 protons and 36 neutrons is what isotope and element?
A)
30/66Zn
B)
36/30Zn
C)
66/30Zn
D)
30/36Zn
17.
What is a photon?
A)
excess energy absorbed by a proton
B)
excess energy emitted from a neutron
C)
excess energy absorbed by an electron
D)
excess energy emitted from an electron
18.
What is the orbital of an electron?
A)
a loop-like planetary trajectory with the lowest probability of finding the electron
B)
a loop-like planetary trajectory with the highest probability of finding the electron
C)
the region of space with the lowest probability of finding the electron
D)
the region of space with the highest probability of finding the electron
19.
How many d orbitals are there?
A)
1
B)
3
C)
5
D)
7
20.
What is the ground state of an electron?
A)
The state in which all electrons are in the lowest possible energy level.
B)
The state in which electrons have been promoted to the lowest possible energy level.
C)
The state in which multiple electrons are located in one of two levels.
D)
The state in which all electrons are in their highest possible energy level.
PROBLEMS:Show all work in solving the following. Be sure to use units of measure and significant figures. Constants:speed of light (c) = 3.0x 108m/s and Planck’s constant (h) = 6.63x10-34J*s
21.
Calculate the weighted average or atomic mass for carbon. C-12 is 98.89% abundant, C-13 is 1.01% abundant, and C-14 is 0.1% abundant.
22.
What is the frequency of a 450nm wavelength?
23.
How much energy is released by a wavelength with a frequency of 6.6x1014 Hz?
24.
SHORT ANSWER/ESSAY: Answer the following in the space provided. Which element has the electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p4?
25.
What is the Heisenberg uncertainty principle?
26.
Write the electron configuration for antimony. (you may use the long or abbreviated form)
27.
The full electron configuration for Carbon is
28. List the contributions to chemistry for 4 of the following people: Gassendi, Proust, Democritus, Chadwick, Goldstein and Thomson. 29. Explain how Rutherford’s experiment supports the following two observations: a. atoms are mostly empty space and b. atoms contain a positively charged central mass.
30. Describe Lavoisier’s experiment. What did he discover and why was it important?
31. Explain how a photon of light is released by an atom. How does this relate to a line spectrum? Why would this be important to someone in the development of fireworks?
32. List the 4 points of Dalton’s atomic theory.
33. What are isotopes? Give an example of their use in medicine.
34. What is the shape of the d orbitals and the s orbitals? 35. How did forensic scientists identify the ashes as either human or other substances?
Chapter 2 Review (please note that the wiki does not allow for the formatting of exponents so 10 to the 4th power looks like 10 4) Multiple choice: circle the best answer
1.
From what material could evidence be found that might yield a conviction of “Tommy Karate” Pitera ?
A)
water samples
B)
soil
C)
grass and leaves
D)
wood samples
2.
What is a characteristic of a chemical change?
A)
a substance melts or freezes
B)
a material evaporates
C)
neither of the above
D)
both of the above
3.
Which of the following does the scientific method utilize?
A)
collecting relevant data
B)
forming a hypothesis
C)
testing the hypothesis
D)
all of the above
.
What is the difference between mass and weight?
A)
All matter has weight, but not all matter has mass.
B)
Weight is a measure of the pull of matter to a scale or measuring device, while mass is a measure of how much matter weighs.
C)
All matter has mass, but only limited amounts have weight.
D)
Weight is a measure of the pull of matter to the earth, while mass is a measure of how much matter is in a sample.
5.
How is weight commonly measured?
A)
with a thermometer
B)
in milliliters
C)
with a scale
D)
in metric units
6.
A scientist knows what constitutes relevant data by
A)
Using common sense
B)
Experience
C)
Judgment
D)
E)
All of the above
None of the above
7.
How many significant figures are there in the number 0.00204?
A)
2
B)
3
C)
4
D)
5
8.
How many significant figures does the number 23.120 have?
A)
3
B)
4
C)
5
D)
6
9.
How many significant figures should the answer to the following calculation have? 18.03 / 9.2 =
A)
1
B)
2
C)
3
D)
4
10.
How many significant figures should the answer to this question have: 14.1 + 3.078 =
A)
2
B)
3
C)
4
D)
5
11.
Which of the following represent three measurements that are the most precise?
A)
1.35, 1.20, and 1.28
B)
1.02, 0.82, and 1.87
C)
1.11, 1.93, and 1.90
D)
1.20, 1.22, and 1.19
12.
A sample has a mass of 0.002 g. Which of the following is the most accurate comparison measurement of it?
A)
0.001 g
B)
0.004 g
C)
0.005 g
D)
0.006 g
SHORT ANSWER: Answer the following in the space provided.
13.
List two examples of chemical properties and two examples of physical properties
14. Identify the type of change that has occurred with the following:
a. charcoal burns _
c. nitroglycerin explodes _
d. copper wire breaks
15.
What is a conversion factor? Give an example.
PROBLEMS:Show all workin solving the following. Be sure to usesignificant figures and units of measurein all answers.
16.
If a material has a density of 4.00 g/mL and a volume of 4.00 mL, what is the mass in g?
17.
a. Have you ever found yourself sitting through a terribly boring class, counting the seconds that remain? If a class has 0.15 hour remaining, how many seconds until the bell rings?
b. How many milliliters are there in 13.500 nL?
18.
Work the following problems and show all work:
a. 17.12 kg=dg
µm/ms
b. 6.2 x10-3 cm/min=µm/ms
19.
You need to earn $100 for homecoming. Your parents tell you that they will pay you $8 per hour to babysit your brother. You need to watch your brother for 45 minutes every Tuesday and Thursday. How many weeks do you need to baby sit your brother? (Remember: you are only babysitting 2 days per week).
20.
Your teacher has given you a piece of metal and expects you to identify it.You are to first make observations. What could you write down about the piece of metal?Next, she gives you the following densities:
Aluminum:2.7g/cm³.
Lead: 11.4 g / ml
Silver: 10.5 gr/cm3
Copper: 8.92 g/cm3
You find the mass of the metal to be 54.3g.
In order to find the volume, you place 30.0 ml of water in a graduated cylinder. Next the metal is gently placed in the cylinder and the new volume is 36.2 ml. Which metal were you given? Show your work to support your answer.__
Chapter 1 Review NOTE: this year the chapter one test will include identification of lab ware - refer to your tools of the trade worksheet. Multiple choice: circle the best answer
1.
What does forensic science deal with?
A)
The application of facts to legal matters
B)
The application of science to legal matters and crime solving
C)
The use of machinery in crime solving
D)
The application of science exclusively to crime solving
2.
Which of the following represents the states of matter from least to most ordered?
A)
liquids, solids, gases
B)
gases, solids, liquids
C)
solids, liquids, gases
D)
gases, liquids, solids
3.
What is constant in a liquid?
A)
volume
B)
shape
C)
both of the above
D)
neither of the above
4.
Pure substances
A)
have a uniform composition and cannot be separated by physical methods
B)
are always elements
C)
are solids in most cases
D)
have a uniform composition that can be separated by physical methods
5.
The smallest unit of an element is a(n) _.
A)
atom
B)
ion
C)
molecule
D)
formula unit
6.
What is the correct atomic symbol for strontium?
A)
Sr
B)
Se
C)
Sb
D)
S
7.
What element name corresponds to the elemental symbol Sb?
A)
antimony
B)
lead
C)
tin
D)
arsenic
8.
What can elements form when they react with other substances?
A)
isotopes
B)
compounds
C)
decay products
D)
mixtures
9.
Which of the following atomic symbols corresponds to manganese?
A)
Mn
B)
Ma
C)
Sb
D)
Si
10.
Which of the following is made from only one element?
A)
aluminum foil
B)
brass
C)
bronze
D)
common table salt
11.
When two or more substances are mixed and evenly distributed so that a sample from any one part of the mixture is chemically identical to a sample from any other part, the mixture is said to be
A)
homogeneous
B)
complete
C)
heterogeneous
D)
molecular
12.
Chromatography is used to
A)
separate mixtures into compounds.
B)
separate compounds into elements.
C)
separate pure substances into atoms.
D)
separate ionic compounds into molecules.
13.
Ru is the element symbol for which element?
A)
rhodium
B)
rubidium
C)
rhenium
D)
ruthenium
14.
The atomic symbols that correspond to sulfur, antimony, and silicon are
A)
S, Sb, and Si
B)
Se, Sb, and Si
C)
S, Se, and Si
D)
S, Sb, and Se
15.
What can all metals conduct?
A)
heat and electricity
B)
heat and air
C)
electricity and atoms
D)
electricity
16.
Which of the following elements are nonmetals?
A)
iron, sulfur, calcium
B)
iron, lead, chlorine
C)
oxygen, bromine, calcium
D)
oxygen, carbon, xenon
17.
What elements are present, and how many atoms of each are in the compound Fe2O3?
A)
2 atoms of iron and 3 atoms of oxygen
B)
2 atoms of fluorine and 3 atoms of oxygen
C)
3 atoms of iron and 2 atoms of oxygen
D)
3 atoms of fluorine and two atoms of oxygen
18.
Matter is a
A)
pure substance
B)
mixture
C)
compound
D)
all of the above
19.
Common table salt, sodium chloride, is an example of what?
A)
a mixture
B)
an element
C)
a homogeneous mixture
D)
a compound
20.
Why was chromatography originally developed?
A)
to separate different particles in mixtures
B)
to separate colored pigments in flowers
C)
to separate different flavors in coffees
D)
to distinguish colored components in coal tar
21.
Alchemy is the study of
A)
changing the color of pennies
B)
changing metal to gold
C)
changing gold to silver
D)
changing silver to gold
22.
Which of the following atomic symbols represent calcium, chromium, and carbon?
A)
Ca, Cr, and C
B)
Cl, Cr, and C
C)
Ca, Cr, and Co
D)
C, Ca, and Co
23.
The following elements are metals:
A)
tin, zinc, and chlorine
B)
hydrogen, zinc, and copper
C)
tin, zinc, and copper
D)
hydrogen, zinc, and chlorine
24.
What is the proper formula for magnesium chloride, which has 1 atom of magnesium, and 2 of chlorine?
A)
MgCl
B)
Mg2Cl
C)
Mg2Cl2
D)
MgCl2
25.
What is baking soda, a substance found in most kitchens?
A)
an element
B)
a compound
C)
a mixture
D)
a solution
Short answer/essay: thoroughly answer each question, using complete sentences where appropriate. Don’t forget to answer all parts.
26.
Explain the difference between metalloids and metals. Where are metals found and where are metalloids found on the periodic table? Which is most abundant?
27.
Explain why observation is considered a critical skill for scientists.
28.
Explain the development of the periodic table.
29.
List 5 safety rules one should follow while doing a lab.
30.
Could we experience heat without matter? why or why not?
31.
Describe the case study and explain what concepts from this unit were used by Agent Rawalt to solve the case.
32.
List and describe the states of matter. Organize them from least to most energy.
33.
Discuss mixtures, identify the types, explain different methods of separating mixtures, and explain how mixtures differ from a pure substance.
34.
You are investigating a crime scene at a museum. You find a note written in black ink by the victim that he had stolen and sold a valuable gold bracelet for $750,000, but he cannot live with what he did. Near the victim, is a pen with black ink. Did the victim write the note? Describe a technique you have learned in this unit to help you decide whether or not the victim wrote the note. (hand writing experts are not available).Also, in a notebook, you find these numbers next to the word bracelet: mass 255g, volume 20mL, density 12.75, and melted in autoclave at 300oC. You know that gold has a density of 19.3g and melts at 1,947oC. Did the victim commit suicide because of his greed or did something else occur? Explain you reasoning.
35.
A new element has been discovered with a density of 1.24 g/cm3 and a melting point of -62oC . Based on the information below answer the following question:
a.the new element should fit between which two elements?
b.would the new element be a metal, nonmetal, or metalloid?
c. describe the hardness of the new element.
Li - density 0.534 g/cm3, melting point 180oC, hardness soft
Na - density 0.971 g/cm3, melting point 98oC, hardness soft
K - density 0.86 g/cm3, melting point 63oC, hardness soft
C - density 2.10 g/cm3, melting point 3550oC, hardness soft, yet brittle Si - density 2.33 g/cm3, melting point 1410oC, hardness brittle
Ge - density 5.32g/cm3, melting point 937oC, hardness fairly brittle
Cl - density 0.00321 g/cm3, melting point -101oC, hardness none
Br - density 3.12g/cm3, melting point -7.2oC, hardness none
I - density 4.93g/cm3, melting point 113.5oC, hardness soft
Ne - density 0.00090g/cm3, melting point -249oC, hardness none
Ar - density 0.00178g/cm3, melting point -189oC, hardness none
Kr - density 0.00374 g/cm3, melting point -156.6oC, hardness none
Chapter 4 part 2 review
Multiple Choice: Circle the best answer.Hg(NO3)2 (aq)+ HCl (aq) → HgCl2(s) + HNO3 (aq)
SHORT ANSWER/ESSAY: Answer the following in the space provided.
P + O2 → P2O5
NaBr + Fe2(CO3)3 → Na2(CO3) + FeBr3
nickel and titanium (I) phosphate form titanium and nickel II phosphate
.
a. the combustion of octane (C8H18) and oxygen
b. the neutralization of HF and CsOH
.
17. Define the following terms and explain how they relate to each other: mole to mole ratio, limiting reactant and theoretical yield.
Problems: Show all work on the math problems. Circle the final answer.
Be sure to use significant figures and units of measure in all answers.
.
2C2H6 + 7 O2 → 4CO2 + 6 H2O
4 Y + 3Br2 → 2 Y2Br3
What is the theoretical yield in grams and which is the limiting reagent?
.
Chapter 4 part I review
Multiple Choice: circle the best answer.SHORT ANSWER/ESSAY: Answer the following in the space provided.
Chapter 3 review
(again, please note that the wiki will not do superscripts or subscripts)Multiple Choice: circle the best answer.
PROBLEMS: Show all work in solving the following. Be sure to use units of measure and significant figures.
Constants: speed of light (c) = 3.0x 108m/s and Planck’s constant (h) = 6.63x10-34J*s
24.
Which element has the electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p4?
29. Explain how Rutherford’s experiment supports the following two observations:
a. atoms are mostly empty space and
b. atoms contain a positively charged central mass.
30. Describe Lavoisier’s experiment. What did he discover and why was it important?
31. Explain how a photon of light is released by an atom. How does this relate to a line spectrum? Why would this be important to someone in the development of fireworks?
32. List the 4 points of Dalton’s atomic theory.
33. What are isotopes? Give an example of their use in medicine.
34. What is the shape of the d orbitals and the s orbitals?
35. How did forensic scientists identify the ashes as either human or other substances?
Chapter 2 Review (please note that the wiki does not allow for the formatting of exponents so 10 to the 4th power looks like 10 4)
Multiple choice: circle the best answer
E)
None of the above
SHORT ANSWER: Answer the following in the space provided.
14. Identify the type of change that has occurred with the following:
a. charcoal burns _
c. nitroglycerin explodes _
d. copper wire breaks
PROBLEMS: Show all work in solving the following. Be sure to use significant figures and units of measure in all answers.
b. How many milliliters are there in 13.500 nL?
a. 17.12 kg = dg
µm/ms
b. 6.2 x10-3 cm/min = µm/ms
Aluminum: 2.7g/cm³.
Lead: 11.4 g / ml
Silver: 10.5 gr/cm3
Copper: 8.92 g/cm3
You find the mass of the metal to be 54.3g.
In order to find the volume, you place 30.0 ml of water in a graduated cylinder. Next the metal is gently placed in the cylinder and the new volume is 36.2 ml. Which metal were you given? Show your work to support your answer.__
Chapter 1 Review NOTE: this year the chapter one test will include identification of lab ware - refer to your tools of the trade worksheet.
Multiple choice: circle the best answer
a.the new element should fit between which two elements?
b.would the new element be a metal, nonmetal, or metalloid?
c. describe the hardness of the new element.
Li - density 0.534 g/cm3, melting point 180oC, hardness soft
Na - density 0.971 g/cm3, melting point 98oC, hardness soft
K - density 0.86 g/cm3, melting point 63oC, hardness soft
C - density 2.10 g/cm3, melting point 3550oC, hardness soft, yet brittle
Si - density 2.33 g/cm3, melting point 1410oC, hardness brittle
Ge - density 5.32 g/cm3, melting point 937oC, hardness fairly brittle
Cl - density 0.00321 g/cm3, melting point -101oC, hardness none
Br - density 3.12 g/cm3, melting point -7.2oC, hardness none
I - density 4.93 g/cm3, melting point 113.5oC, hardness soft
Ne - density 0.00090 g/cm3, melting point -249oC, hardness none
Ar - density 0.00178 g/cm3, melting point -189oC, hardness none
Kr - density 0.00374 g/cm3, melting point -156.6oC, hardness none